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JIPMER 2004
Exam
JIPMER
Year
2004
Subject
Chemistry
Chapter
Electrochemistry

JIPMER 2004 · Chemistry · Electrochemistry

Two metals 'A' and 'B' have E_ red ^ value equal to 0.36 V and 1.23...

Two metals 'A' and 'B' have \mathrm{E}_{\text{red }^{\circ}valueequalto0.36Vand1.23V.Whatwillbethecorrectcellequation?value equal to 0.36 V and 1.23 V . What will be the correct cell equation?

Options

  1. AA+B2+⟶A2++B\mathrm{A}+\mathrm{B}^{2+} \longrightarrow \mathrm{A}^{2+}+\mathrm{B}
  2. BA2++B⟶A+B2+\mathrm{A}^{2+}+\mathrm{B} \longrightarrow \mathrm{A}+\mathrm{B}^{2+}
  3. CBoth (1) and (2)
  4. DNone of the above

Correct answer

A. A+B2+⟶A2++B\mathrm{A}+\mathrm{B}^{2+} \longrightarrow \mathrm{A}^{2+}+\mathrm{B}

Step-by-step solution

From Ered ∘E_{\text{red }}^{\circ}. values, it is clear that AA is more electropositive than BB (as it has lesser E∘red E^{\circ}{ }_{\text{red }} ), hence it can replace BB from its salt solution and act as anode in galvanic cell. Hence, correct cell equation will be: A+B2+⟶A2++BA+B^{2+} \longrightarrow A^{2+}+B
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